Objective:
The purpose of this experiment was to produce aspirin using salicylic acid and acetic acid.
Experimental Section:
There were four parts to this lab. The first experiment, was synthesizing. A 600 ml beaker was filled with water and placed on the hot plate until it boiled. The measurement was .995g. The salicylic acid was transferred into a 125 ml Erlenmeyer flask and the acetic was given by the lab instructor. Three drops of 85% phosphoric acid. While swirling and mixing more was added and then clamp onto the sing stand in the boiling water for 8 minutes. 1 mL drops of water was added in the flask. The second experiment, was crystallization. After the reaction subsided 20 mL of water was added and removed from the ring stand
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It was placed in an ice bath for 10 minutes with occasionally swirls. The third experiment, was Filteration. The vacuum filtration apparatus, the filter flask and the aspirator trap bottle was set up for this section. The crude aspirin was collected by the vacuum filtration. The sample was poured in the Buchner funnel and a about 5 mL of water was in the flask to get the last few of crystal out of the flask. After the crude aspirin dry in the beaker it weighed about 2.575 without the beaker. The final experiment, was purification. The crude aspirin was tranfer into a 125 mL Erlenmeyer flask with 3 mL of ethanol and warm on the hot plate until the aspirin dissolve. Fiver portions of about 3 mL of water was added in increments and cooled in an ice bath for about 10 minutes. After a new filter paper was add and the aspirin was placed in while the vacuum filtration was on and about 6 mL was poured in to get the last amount of …show more content…
Also, one was more moist than the other. The second reactant was whiter than the first reactant. Also, the second reactant dried faster than the first reactant.
Question 4: The weight of the crude aspirin was 2.575 g and the weight of the purified aspirin was .0316 g. The crude aspirin was cloudy than the purified aspirin. The purified was whiter than the crude aspirin. In the end, the purified aspirin had a more darker/ boler color than the crude aspirin. The explanation for the difference are the addition of 3 mL of ethanol while purifying the aspirin.
Conclusion:
The objective was met because by completing each experiment aspirin was produce. Many things were learned from this experiment. Making aspirin was very hard, it was a long process to produce aspirin. Also, getting a 100 % yield was very hard because residue may be left from the step before or a may beaker may break and some sample may lose. Even though this lab took a very long time to complete it was very fun to see the
The experiment was not a success, there was percent yield of 1,423%. With a percent yield that is relatively high at 1,423% did not conclude a successful experiment, because impurities added to the mass of the actual product. There were many errors in this lab due to the product being transferred on numerous occasions as well, as spillage and splattering of the solution. Overall, learning how to take one product and chemically create something else as well as how working with others effectively turned out to be a
A: The reaction with water and vinegar was the most useful in this experiment. The physical properties were very self explanatory because the texture of the powders was all different expect icing sugar and cornstarch. Also the Ph levels were very similar of six and seven for corn starch and icing sugar respectively. d) Q: How confident do you feel about your identification of the
The procedure of the lab on day one was to get a ring stand and clamp, then put the substance in the test tube. Then put the test tube in the clamp and then get a Bunsen burner. After that put the Bunsen burner underneath the test tube to heat it. The procedure of the lab for day two was almost exactly the same, except the substances that were used were different. The
Looking at my results, I can see that I only obtained 86.6% of aspirin. this is not the highest percentage that it could be. I probably lost some aspirin when I had to re-filtered the solution multiple times, or when I had to weigh a new beaker and maybe not all of it got transferred over to the new beaker, or maybe I didn’t get all of the aspirin crystals off of the paper towel and into the beaker. Regardless, of where the aspirin sample was lost, I obtained a 86.6% of aspirin from this
Aspirin contains the substance acetylsalicylic acid (ASA), which can relieve inflammation, fever, pain, and known as a “blood thinner”. Aspirin was not officially trademarked until March 6, 1899 when the Imperial Office of Berlin made it official. It has been used for the last 110 years, but its natural form, salicylic acid has been around for thousands by Egyptians, Greeks, and Romans. Aspirin is available in over 80 countries and known as the best non-prescription drug. The most common use of aspirin is to cure headaches and use it as a pain reliever, but aspirin is known to prevent heart attack and strokes. It was first proposed in 1940, but wasn’t confirmed until 1970 when doctors would recommend taking aspirin daily [1].
Planning Firstly here is a list of equipment I used. Boiling tubes Weighing scales Knife Paper towels 100% solution 0% solution (distilled water) measuring beakers potato chips Cork borer. We planned to start our experiment by doing some preliminary work. We planned to set up our experiment in the following way.
The purpose of this experiment was to learn and preform an acid-base extraction technique to separate organic compounds successfully and obtaining amounts of each component in the mixture. In this experiment, the separation will be done by separatory funnel preforming on two liquids that are immiscible from two layers when added together. The individual components of Phensuprin (Acetylsalicylic acid, Acetanilide, and Sucrose as a filler) was separated based upon their solubility and reactivity, and the amount of each component in the mixture was obtained. Also, the purity of each component will be determined by the melting point of the component.
For this experiment we have to use physical methods to separate the reaction mixture from the liquid. The physical methods that were used are filtration and evaporation. Filtration is the separation of a solid from a liquid by passing the liquid through a porous material, such as filter paper. Evaporation is when you place the residue and the damp filter paper into a drying oven to draw moisture from it by heating it and leaving only the dry solid portion behind (Lab Guide pg. 33.).
One possible source of experimental error could be not having a solid measurement of magnesium hydroxide nor citric acid. This is because we were told to measure out between 5.6g-5.8g for magnesium hydroxide and 14g-21g for citric acid. If accuracy measures how closely a measured value is to the accepted value and or true value, then accuracy may not have been an aspect that was achieved in this lab. Therefore, not having a solid precise measurement and accurate measurement was another source of experimental error.
* It was almost impossible to tell when the Alka-Seltzer tablet had dissolved, each time the experiment was done. This was a huge problem for the experiment as this could have totally caused problems to the experiment. A special type of detector apparatus, which bleeped when the correct amount of Alka-Seltzer tablet dissolved, could improve this, each time the experiment was done.
The conical vial was placed in a small beaker and allowed to cool to room temperature. The mixture was Cooled thoroughly in an ice bath for 15-20 minutes and crystals collected by vacuum filtration on a Hirsch funnel. The vial was rinsed with about 5 mL of ice water and transferred into to the Hirsch funnel and again washed with two additional 5mL portions of ice water. Crystals were dried for 5-10 minutes by allowing air to be drawn through them while they remained on the Hirsch funnel. The product was transferred to a watch glass plate and allow the crystals to dry in air. Crude acetaminophen product was weighed and set aside a small sample for a melting point determination and a color comparison after the next step. Calculation of the percentage yield of crude acetaminophen (MW = 151.2). was done and recorded in the lab notebook.
Analysis of Aspirin Tablets Aim --- To discover the percentage of acetylsalicylic acid in a sample of aspirin tablets. ----------------------------------------------------------------- In order to do this, the amount of moles that react with the sodium hydroxide must be known. This is achieved by using the method of back titration.
The first experiments investigate the order of reaction with respect to the reactants; hydrogen peroxide, potassium iodide and sulphuric acid by varying the concentrations and plotting them against 1/time. An initial rate technique is used in this experiment so ‘the rate of reaction is inversely proportional to time.’ To find the order of reaction in respect to the reactants, 1/time is plotted against the concentration of Hydrogen Peroxide using the equation:
An error that occurred in the experiment was during the ceric nitrate test because solution 4 should have produced a color change. During a base hydrolysis of aspartame, aspartic acid, phenylalanine and methanol are produced, therefore the ceric nitrate test should have been a positive for alcohol. A reason that this could have shown a negative result is because methanol is a volatile substance and it could have evaporated out, which would have caused a negative ceric nitrate test
Firstly, we need to keep the chemical at a constant concentration. So, in this experiment we have chosen to keep hydrochloric acid at a constant concentration (5cm3). We could have, however, used Sodium Thiosulphate as a constant, but we had chosen to use Hydrochloric acid. Next, we must make sure that the solution is kept at a constant volume throughout the experiment. If the volume is different, then it could give different results if it was at a constant volume.